1. Solutions, Acids, and Bases Ch. 15 and 16

2. Solution Solute-what is BEING dissolved the lesser substance Solvent-what is DOING the dissolving the greater substance Solutes and solvents can be any state of matter: solid, liquids or gases

3. Examples of solutions Solid-solid solution: Bronze, 18 K gold; pewter Solid-liquid solution: Saline solution, kool-aid Liquid-gas solution: Coke Gas-gas solution: Air Liquid- liquid solution: Alcohol

4. Solubility The ability of a substance to dissolve another substance You may see this solubility chart on your GHSGT or SAT: The solubility of which substance is most affected by an increase in temperature?

5. More surface area (crush) Shake or stir Increase temperature Not all substance dissolve. Some are Soluble, Insoluble, or partly soluble To increase RATE of dissolving:

6. Concentration: the ratio of solute to solvent Dilute: more solvent than solute (“watered down”) Concentrated: more solute than solvent (orange juice from concentrate; Pine Sol)

7. Concentration of solutions We used solutions of different concentrations in labs: 1 M HCl; 6 M NaOH;.5 M Pb(NO 3 ) 2 The higher the number, the more concentrated the solution Unit of concentration is Molar (M) 1 Molar solution has 1 mole of solute dissolved in 1 Liter. 6 Molar solution has 6 moles of solute dissolved in 1 Liter

8. Types of solutions Saturated-As much solute as possible is dissolved at that temperature. Kool-aid, chocolate milk Unsaturated-More solute can still dissolve in the solution. Supersaturated- a solution that has dissolved more solute than usual by increasing the temperature. Making jello; or making candy. (You have to heat the water first to dissolve the sugar.)

9. Solubility Curve Be able to read a graph! Saturated is on the line. Unsaturated is under the line Supersaturated is above the line. Supersaturated Saturated Unsaturated

10. Acids and Bases Are measured by the H + ion concentration using the pH scale.

11. pH Scale pH means –log of H + concentration scale ranges from 0-14; every step away from seven is a power of ten more acidic or basic 7 is neutral: H + = OH - concentration

12. Acids Produce H + ions in solution: H + + H 2 O -> H 3 O + (hydronium ion) Properties of acids: Taste sour Corrosive Conduct electricity Turns litmus paper RED pH of 0 - 6.9 (pH means the concentration of H + ions)

13. Common Acids Strong acids (strong electrolytes) HCl; HNO 3 ; H 2 SO 4 HF Lemon juice Gastric acid Weak Acids (weak electrolytes) Vinegar Carbonic acid Citric acids

14. Bases Produce OH - ions in solution: Properties of bases: Taste bitter Feels slippery Corrosive Conduct electricity Turns litmus paper BLUE pH of 7.1 - 14

15. Common Bases Strong bases (strong electrolytes) Drano NaOH; KOH Weak Bases (weak electrolytes) Deodorant Ammonia Soaps Shampoos antacids

16. Neutralization Reactions Acid + base = forms a salt and water A base neutralizes an acid and vice versa. An antacid (TUMS, rolaids) neutralizes stomach acid Deodorant neutralizes acidic sweat